Download Mass Spectrometry (MS)

William H. Brown
Christopher S. Foote
Brent L. Iverson
Eric Anslyn
http://academic.cengage.com/chemistry/brown
Chapter 14
Mass Spectrometry
William H. Brown • Beloit College
14-1
Mass Spectrometry (MS)
 An
analytical technique for measuring the massto-charge ratio (m/z) of ions in the gas phase.
• Mass spectrometry is our most valuable analytical tool
for determining accurate molecular masses.
• Also can give information about structure.
• Proteins can now be sequenced by MS.
14-2
Mass Spectrometry (MS)
 Schematic
of an electron ionization mass
spectrometer (EI-MS).
14-3
A Mass Spectrometer
A
mass spectrometer is designed to do three
things
• Convert neutral atoms or molecules into a beam of
positive (or rarely negative) ions.
• Separate the ions on the basis of their mass-to-charge
(m/z) ratio.
• Measure the relative abundance of each ion.
14-4
A Mass Spectrometer
 Electron
Ionization MS
• In the ionization chamber, the sample is
bombarded with a beam of high-energy electrons.
• Collisions between these electrons and the
sample result in loss of electrons from sample
molecules and formation of positive ions.
H
H C H + e
H
+
H
+2 e
H C H
H
Molecular ion
(a radical cation)
14-5
Molecular Ion
 Molecular
ion (M): A radical cation formed by
removal of a single electron from a parent
molecule in a mass spectrometer.
 For our purposes, it does not matter which
electron is lost; radical cation character is
delocalized throughout the molecule; therefore,
we write the molecular formula of the parent
molecule in brackets with
• a plus sign to show that it is a cation.
• a dot to show that it has an odd number of electrons.
14-6
Molecular Ion
• At times, however, we find it useful to depict the
radical cation at a certain position in order to better
understand its reactions.
CH3 CH2 OCH( CH3 ) 2 .
CH3 CH2 OCH( CH3 ) 2
14-7
Mass Spectrum
 Mass
spectrum: A plot of the relative abundance
of ions versus their mass-to-charge ratio.
 Base peak: The most abundant peak.
• Assigned an arbitrary intensity of 100.
 The
relative abundance of all other ions is
reported as a % of abundance of the base peak.
14-8
MS of dopamine
• a partial mass spectrum of dopamine showing all
peaks with intensity equal to or greater than 0.5% of
the base peak.
14-9
MS of Dopamine
• The number of peaks in the mass spectrum of
dopamine is given here as a function of detector
sensitivity.
HO
HO
NH2
Peak Intensity
Relative to
Bas e Peak
> 5%
> 1%
> 0.5%
> 0.05%
Number
of Peaks
Recorded
8
31
45
120
14-10
Other MS techniques
 What
we have described is called electron
ionization mass spectrometry (EI-MS).
 Other mass spectrometry techniques include
•
•
•
•
fast atom bombardment (FAB).
matrix-assisted laser desorption ionization (MALDI).
chemical ionization (CI).
electrospray ionization (ESI).
14-11
Resolution
 Resolution:
A measure of how well a mass
spectrometer separates ions of different mass.
• Low resolution: Refers to instruments capable of
separating only ions that differ in nominal mass; that
is ions that differ by at least 1 or more atomic mass
units (amu).
• High resolution: Refers to instruments capable of
separating ions that differ in mass by as little as 0.0001
amu.
14-12
Resolution
• C3H6O and C3H8O have nominal masses of 58 and 60,
and can be distinguished by low-resolution MS.
• C3H8O and C2H4O2 both have nominal masses of 60.
• distinguish between them by high-resolution MS.
Molecular N ominal Precise
Formula
Mass
Mas s
C3 H8 O
60
60.05754
C2 H4 O2
60.02112
60
14-13
Isotopes
• Virtually all
elements
common to
organic
compounds
are mixtures
of isotopes.
Atomic
Element w eigh t Isotope
hydrogen 1.0079 1H
2
H
carbon
12.011 12
C
13
C
nitrogen 14.007 14 N
15
N
16
oxygen
15.999
O
18
O
32
su lfu r
32.066
S
34
S
ch lorine 35.453 3 5Cl
37
Cl
bromine 79.904 79Br
81
Br
Mas s Relative
(amu ) A bun dance
1.00783 100
2.01410
0.016
12.0000 100
13.0034
1.11
14.0031
100
15.0001
0.38
15.9949 100
17.9992
0.20
31.9721 100
33.9679
4.40
34.9689 100
36.9659
32.5
78.9183 100
80.9163
98.0
14-14
Isotopes
• Carbon, for example, in nature is 98.90% 12C and 1.10%
113C.
• There are 1.11 atoms of carbon-13 in nature for every
100 atoms of carbon-12.
1.10
C x 100 1 2
98.90 C
13
x 100
= 1.11 atoms
13
C per 100 atoms
12
C
14-15
M+2 and M+1 Peaks
 The
most common elements giving rise to
significant M + 2 peaks are chlorine and bromine.
• Chlorine in nature is 75.77% 35Cl and 24.23% 37Cl.
• A ratio of M to M + 2 of approximately 3:1 indicates the
presence of a single chlorine in a compound, as seen
in the MS of chloroethane.
14-16
M+2 and M+1 Peaks
• Bromine in nature is 50.7% 79Br and 49.3% 81Br.
• A ratio of M to M + 2 of approximately 1:1 indicates the
presence of a single bromine atom in a compound, as
seen in the MS of 1-bromopropane.
14-17
M+2 and M+1 Peaks
 Sulfur
is the only other element common to
organic compounds that gives a significant M + 2
peak
•
32S
= 95.02% and 34S = 4.21%
 Because
M + 1 peaks are relatively low in
intensity compared to the molecular ion and
often difficult to measure with any precision, they
are generally not useful for accurate
determinations of molecular weight.
14-18
Fragmentation of the Molecular Ion
 To
attain high efficiency of molecular ion
formation and give reproducible mass spectra, it
is common to use electrons with energies of
approximately 70 eV [6750 kJ (1600 kcal)/mol].
• This energy is sufficient not only to dislodge one or
more electrons from a molecule, but also to cause
extensive fragmentation.
• These fragments may be unstable as well and, in turn,
break apart to even smaller fragments.
14-19
Fragmentation of M
 Fragmentation
of a molecular ion, M, produces a
radical and a cation.
• Only the cation is detected by MS.
A-B
+
•
Molecular ion
(a radical cation)
A• +
B+
Radical
Cation
+
A
+ • B
Cation
Radical
14-20
Fragmentation of M
A
great deal of the chemistry of ion
fragmentation can be understood in terms of the
formation and relative stabilities of carbocations
in solution.
• Where fragmentation occurs to form new cations, the
mode that gives the most stable cation is favored.
• The probability of fragmentation to form new
carbocations increases in the order.
CH3
+
2°
3°
< 1° < 1° allylic < 2° allylic < 3° allylic
3° benzylic
1° benzylic
2° benzylic
14-21
Interpreting a mass spectrum
 The
only elements to give significant M + 2 peaks
are Cl and Br.
• If no large M + 2 peak is present, these elements are
absent.
 Is
the mass of the molecular ion odd or even?
 Nitrogen Rule: If a compound has
• zero or an even number of nitrogen atoms, its
molecular ion will have an even m/z value.
• an odd number of nitrogen atoms, its molecular ion
will have an odd m/z value.
14-22
Alkanes
 Fragmentation
tends to occur in the middle of
unbranched chains rather than at the ends.
 The difference in energy among allylic, benzylic,
3°, 2°, 1°, and methyl cations is much greater
than the difference among comparable radicals.
• Where alternative modes of fragmentation are
possible, the more stable carbocation tends to form in
preference to the more stable radical.
14-23
Alkanes
• Mass spectrum of octane.
14-24
Alkanes
• Mass spectrum of 2,2,4-trimethylpentane.
14-25
Alkanes
• Mass spectrum of methylcyclopentane.
14-26
Alkenes
 Alkenes
characteristically
• show a strong molecular ion peak.
• cleave readily to form resonance-stabilized allylic
cations.
+
[CH2=CHCH2 CH2 CH3 ] •
CH2 =CHCH2 + +
• CH2 CH3
14-27
Cyclohexenes
• Cyclohexenes give a 1,3-diene and an alkene, a
process that is the reverse of a Diels-Alder
reaction (Chapter 24).
CH3
+
•
CH3
H3 C
C
H3 C
C
+
•
+
CH2
CH2
Limon ene
(m/z 136)
A neu tral d iene
(m/z 68)
A radical cation
(m/z 68)
14-28
Alkynes
 Alkynes
typically
• show a strong molecular ion peak.
• cleave readily to form the resonance-stabilized
propargyl cation or substituted propargyl cations.
+
+
3-Propynyl cation
(Propargyl cation)
HC C-CH2
HC C=CH2
14-29
Alcohols
 One
of the most common fragmentation patterns
of alcohols is loss of H2O to give a peak which
corresponds to M-18.
 Another common pattern is loss of an alkyl
group from the carbon bearing the OH to give a
resonance-stabilized oxonium ion and an alkyl
radical.
R'
•
+
H
R C O
••
R"
Molecular ion
(a radical cation)
R• +
A radical
+
+
••
R' -C ••O H
R' -C= O- H
R"
R"
A resonance-stabilized
oxonium ion
14-30
Alcohols
• Mass spectrum of 1-butanol.
14-31
Aldehydes and Ketones
 Characteristic
fragmentation patterns are
• cleavage of a bond to the carbonyl group (-cleavage).
• McLafferty rearrangement.
O
+
+
•
O
-cleavage
m/z 128
+
•
m/z 43
CH3 •
+
O
+
m/z 113
H
O
Molecular ion
m/z 114
+
•
McLafferty
rearrangement
H
+
O
+
•
m/z 58
14-32
Aldehydes and Ketones
• Mass spectrum of 2-octanone.
14-33
Carboxylic Acids
 Characteristic
fragmentation patterns are
• -cleavage to give the ion [CO2H]+ with m/z 45.
• McLafferty rearrangement.
O
-cleavage
OH
•
+
O= C-O- H
m/z 45
Molecular ion
m/z 88
H
O
OH
Molecular ion
m/z 88
+
•
+
McLafferty
rearrangement
H
+
+
•
O
OH
m/z 60
14-34
Carboxylic Acids
• Mass spectrum of butanoic acid.
14-35
Esters
 -cleavage
and McLafferty rearrangement
+
•
O
OCH3
-cleavage
O
+
m/z 71
+
+
•
O
OCH3
Molecular ion
m/z 102
• OCH 3
O
Molecular ion
m/z 102
H
+
McLafferty
rearrangement
H
+
+
OCH3
m/z 59
+
•
O
OCH3
m/z 74
14-36
Esters
• Mass spectrum of methyl butanoate.
14-37
Aromatic Hydrocarbons
• Most show an intense molecular ion peak.
• Most alkylbenzenes show a fragment ion of m/z 91.
H
+•
CH3
Toluene radical
cation
- H•
H
H
H Tropylium cation
(m/z 91)
+
H
H
H
14-38
Amines
 The
most characteristic fragmentation pattern of
1°, 2°, and 3° aliphatic amines is -cleavage.
CH3
CH3 - CH- CH 2 -CH 2 -N H2
-cleavage
CH3
CH3 - CH- CH 2
•
+
+ CH2 = N H2
m/z 30
14-39
Mass Spectrometry
End Chapter 14
14-40